The process in which no heat enters or leaves the system is termed as

$A$ gas is compressed adiabatically until its temperature is doubled. The ratio of its final volume to initial volume will be

An ideal gas at pressure $p$ is adiabatically compressed so that its density becomes twice that of the initial. If $\gamma = \frac{c_p}{c_v} = \frac{7}{5}$,then the final pressure of the gas is:

An ideal gas at $27^{\circ} C$ is compressed adiabatically to $8/27$ of its original volume. If the ratio of specific heats is $\gamma = 5/3$,then the rise in temperature of the gas is: (in $K$)

$A$ sample of $1$ mole of gas at temperature $T$ is adiabatically expanded to double its volume. If the adiabatic constant for the gas is $\gamma = \frac{3}{2}$,then the work done by the gas in the process is:

$A$ polyatomic gas $(\gamma = 4/3)$ is compressed to $(1/8)^{\text{th}}$ of its initial volume adiabatically. If its initial pressure is $P_0$,what will be its new pressure (in $P_0$)?